Question

The pH of \(0.01\) M aqueous aniline solution at \(298\) K is \(8.3\). Its degree of dissociation \((\alpha)\) is \[ (K_b\text{ of aniline}=4\times10^{-10}; \ \text{antilog}(0.7)=5.0; \ \text{antilog}(0.3)=2.0; \ \text{antilog}(0.4)=2.5) \]

• A. \(10^{-4}\)
• B. \(4\times10^{-4}\)
• C. \(1.5\times10^{-4}\)
• D. \(2\times10^{-4}\)

Hint:

For a weak base, \[ \boxed{ [\mathrm{OH^-}]=C\alpha. } \] First calculate \[ \boxed{\mathrm{pOH}=14-\mathrm{pH}} \] and then obtain \([\mathrm{OH^-}]\).

Answer 1

The Correct Option is D